Select all the choices that have a formation enthalpy of zero. A. Oxygen gas, O2(g) B. Nitrogen gas, N2(g) C. Atomic chlorine, Cl(g) D. Magnesium metal, Mg(s) E. Carbon monoxide, CO(g)

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Write an equation which represents the standard enthalpy of formation reactions. [You must include the states of matter for each atom or compound.] a. Ca(NO 3)2 (s), b. CH3OH (1), c. NaClO4 (s)

D. All of the statements are false. 2NO + 0₂ → NO, A, H° = 90.25 kJ/mol NO₂, AH° = 33.18 kJ/mol → 2NO₂ For numbers 3-4: Consider the data given. 3. What is the value of the standard enthalpy of reaction (kJ/mol)? A. 57.07 C. 114.14 B. -57.07 D. -114.14 4. What is the value of the standard enthalpy of reaction (kJ/mol) of the decomposition of NO2? A. 57.07 C. 114.14 D. -114.14 B. -57.07

Cl2 (g) + H2 (g) → 2 HCl (g)                ΔH0rxn = ‒184.6 kJ 9.   What is the formation reaction of HCl (g)?  Group of answer choices A.No answer text provided. B.2 HCl (g) → Cl2 (g) + H2 (g) C.½ Cl2 (g) + ½ H2 (g) → HCl (g) D.HCl (g) → ½ Cl2 (g) + ½H2 (g) E.Cl2 (g) + H2 (g) → 2 HCl (g)

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1100. g of water (see sketch at right). thermometer stirrer First, a 5.500 g tablet of benzoic acid (C,H,CO, H) is put into the "bomb" and burned completely in an excess of water oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed insulation to rise from 15.00 °C to 42.56 °C over a time of 10.3 minutes. Next, 5.720 g of acetaldehyde (C2H,O} are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 15.00 °C to 40.53 °C. chemical reaction "bomb" Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: A "bomb" calorimeter. 2C,H,0(g) + 50, (g) 4CO, (g) + 4H,0 (g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note…

2. a. Determine the standard heat of formation, AH for the following reaction using the Data from the Table. C3H12 ) + 802(g) → 5CO2 + 6H₂O b. State whether the reaction is exothermic or endothermic. Explain. c. Rewrite the equation as thermochemical equations in two different ways to include the heat calculated in (2a). d. Draw a detail Energy Diagram representing the thermochemical equation in Ⓒ illustrating the the reactants and products and their positions.

6. Calculate the enthalpy change of the following reaction between nitrogen gas and oxygen gas, given thermochemical equations (1), (2), (3). 2N2(g) + 502(g) → 2N₂O(g) 2H2(g) + O2(g) → 2H₂O) N₂O + H₂O → 2HNO30) 0₂(g) + ₂H₂(g) → HNO 3 (1) + (1) (2) (3) 1/2N2(8) AH = -572 kJ AH = -77 kJ| AH-174 kJ

The enthalpy change for a chemical reaction is the sum of the energy consumed in breaking bonds and the energy released during bond formation. One way to determine the overall energy change for a chemical reaction is to apply Hess’s law to add together a group of reactions which can be arranged such that the chemical equations, when combined, give the overall equation we are trying to characterize.     a. Write a balanced chemical equation for the combustion of gaseous propane in gaseous oxygen to produce gaseous carbon dioxide and liquid water.      C3​H8​(g)+    O2​(g) ---->CO2​(g)+     H2​O(g)   b. Combine the following equations to determine the enthalpy change for the combustion of 1 mole of propane. Assume that solid carbon is graphite.  3C(s,graphite)+4H2​(g)--->C3​H8​(g) ΔHo = -103.8 kJ/mol   C(s,graphite)+O2​(g)--->CO2​(g) ΔHo= -393.5 kJ/mol   H2​(g)+1/2​ O2​(g)--->H2​O(g) ΔHo= -285.8 kJ/mol      kJ/mol…